   # You have two 500.0-mL aqueous solutions. Solution A is a solution of a metal nitrate that is 8.246% nitrogen by mass. The ionic compound in solution B consists of potassium, chromium, and oxygen; chromium has an oxidation state of + 6 and there are 2 potassiums and 1 chromium in the formula. The masses of the solutes in each of the solutions are the same. When the solutions are added together, a blood-red precipitate forms. After the reaction bas gone to completion, you dry the solid and find that it has a mass of 331.8 g. a. Identify the ionic compounds in solution A and solution B. b. Identify the blood-red precipitate. c. Calculate the concentration (molarity) of all ions in the original solutions. d. Calculate the concentration (molarity) of all ions in the final solution. ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 6, Problem 147MP
Textbook Problem
296 views

## You have two 500.0-mL aqueous solutions. Solution A is a solution of a metal nitrate that is 8.246% nitrogen by mass. The ionic compound in solution B consists of potassium, chromium, and oxygen; chromium has an oxidation state of + 6 and there are 2 potassiums and 1 chromium in the formula. The masses of the solutes in each of the solutions are the same. When the solutions are added together, a blood-red precipitate forms. After the reaction bas gone to completion, you dry the solid and find that it has a mass of 331.8 g.a. Identify the ionic compounds in solution A and solution B.b. Identify the blood-red precipitate.c. Calculate the concentration (molarity) of all ions in the original solutions.d. Calculate the concentration (molarity) of all ions in the final solution.

a)

Interpretation Introduction

Interpretation: The ionic compounds in solution A and B has to be identified.

Concept Introduction: When two soluble solutions are mixed together, an insoluble salt formation occurs called as precipitate. These precipitates fall out of the solution and the reactions are called as precipitation reaction.

Concentration of solution can be defined in terms of molarity as moles of solute (in grams) to the volume of solution (in litres). The concentration of solution can be calculated by,

Concentration(M)=Molesofsolute(g)Volumeofsolution(L)

### Explanation of Solution

Given:

Record the given data

Volume of two aqueous solution   = 500.0mL

Mass percent of Nitrogen in solution A = 8.246%

Mass of precipitate   = 331.8g

The volume of two aqueous solutions along with mass percent of Nitrogen in solution A of metal nitrate and mass of precipitate are recorded as shown above.

To identify the ionic compound in solution A

Molecular mass of oxygen = 16.00g

Molecular mass of nitrogen = 14.01g

Compound A contains metal nitrate M(NO3)x

Assuming the mass of metal nitrate is M(NO3)x = 100.0g

The moles of oxygen is calculated using

Molesofoxygen=8.246g48.00gO14.01gN=28.25gO

Thus, the mass of nitrate = 8.246+28.25g=36.50g(ifx=1)

Case 1:

x=1:massofM=100.00-36.50g=63.50g

MolM=molN=8.246g14.01g/mol=0.5886mol

MolarmassofmetalM=63.50g0.5886mol=107

b)

Interpretation Introduction

Interpretation: The blood-red precipitate has to be identified.

Concept Introduction: When two soluble solutions are mixed together, an insoluble salt formation occurs called as precipitate. These precipitates fall out of the solution and the reactions are called as precipitation reaction.

Concentration of solution can be defined in terms of molarity as moles of solute (in grams) to the volume of solution (in litres). The concentration of solution can be calculated by,

Concentration(M)=Molesofsolute(g)Volumeofsolution(L)

c)

Interpretation Introduction

Interpretation: The concentration of original solution has to be calculated.

Concept Introduction: When two soluble solutions are mixed together, an insoluble salt formation occurs called as precipitate. These precipitates fall out of the solution and the reactions are called as precipitation reaction.

Concentration of solution can be defined in terms of molarity as moles of solute (in grams) to the volume of solution (in litres). The concentration of solution can be calculated by,

Concentration(M)=Molesofsolute(g)Volumeofsolution(L)

d)

Interpretation Introduction

Interpretation: The concentration of final solution has to be calculated.

Concept Introduction: When two soluble solutions are mixed together, an insoluble salt formation occurs called as precipitate. These precipitates fall out of the solution and the reactions are called as precipitation reaction.

Concentration of solution can be defined in terms of molarity as moles of solute (in grams) to the volume of solution (in litres). The concentration of solution can be calculated by,

Concentration(M)=Molesofsolute(g)Volumeofsolution(L)

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